How much hydrogen is required to produce iron when interacting with 25.52 g of Pe3O4

How much hydrogen is required to produce iron when interacting with 25.52 g of Pe3O4 containing 30% impurities.

The reduction reaction of iron oxide with hydrogen is described by the following chemical reaction equation:

Fe3O4 + 4H2 = 3Fe + 4H2O;

According to the coefficients of the chemical reaction, four moles of hydrogen are required for one mole of iron oxide.

Let’s find the amount of the substance in 25.52 grams of iron oxide.

M Fe3O4 = 56 x 2 + 16 x 4 = 176 grams / mol;

N Fe3O4 = 25.52 / 176 = 0.145 mol;

The amount of hydrogen will be 0.145 x 4 = 0.58 mol.

One mole of ideal gas under normal conditions takes a volume of 22.4 liters.

V H2 = 0.58 x 22.4 = 12.992 liters;